Choose the correct statement(s):

Options

A. `H^(+)` is the smalest size cation in the periodic table.
B. van der waals' radius of chlorine is more than covalent radius
C. ionic mobility of hydrated `Li^(+)` is greater than that of hydrated `Na^(+)`.
D. He atom is having highest I.E. in the periodic state

Answer

To solve the question "Choose the correct statement(s)", we will analyze each statement provided in the video transcript step by step.

### Step 1: Analyze the first statement
**Statement:** H⁺ is the smallest size cation in the periodic table.

**Explanation:**
- Hydrogen (H) has an atomic number of 1, which means it has one electron. When it loses this electron to form H⁺, it has no electrons left.
- Therefore, H⁺ is indeed the smallest cation because it has no electron cloud, making its size effectively zero.

**Conclusion:** This statement is correct.

### Step 2: Analyze the second statement
**Statement:** The Van der Waals radius of chlorine is more than its covalent radius.

**Explanation:**
- The Van der Waals radius is defined as half the distance between two non-bonded atoms in a molecule, while the covalent radius is half the distance between two bonded atoms.
- Since Van der Waals forces are weaker than covalent bonds, the distance between non-bonded atoms (Van der Waals radius) is greater than that between bonded atoms (covalent radius).

**Conclusion:** This statement is correct.

### Step 3: Analyze the third statement
**Statement:** Ionic mobility of hydrated Li⁺ is greater than that of hydrated Na⁺.

**Explanation:**
- Ionic mobility refers to the ability of an ion to move through a solution.
- Li⁺ is smaller than Na⁺, which means it can interact more effectively with water molecules when hydrated.
- However, when hydrated, the mobility of ions generally decreases due to the mass of the water molecules surrounding them.
- Therefore, although Li⁺ is smaller, the statement that its ionic mobility is greater than that of Na⁺ when both are hydrated is incorrect.

**Conclusion:** This statement is incorrect.

### Step 4: Analyze the fourth statement
**Statement:** Helium atom has the highest ionization energy in the periodic table.

**Explanation:**
- Ionization energy is the energy required to remove an electron from an atom.
- Helium has a complete outer shell (1s²), which means it has a strong attraction between the nucleus and its electrons.
- As a result, it requires a significant amount of energy to remove an electron from helium, making it have the highest ionization energy among all elements.

**Conclusion:** This statement is correct.

### Final Conclusion
The correct statements are:
- H⁺ is the smallest size cation in the periodic table.
- The Van der Waals radius of chlorine is more than its covalent radius.
- Helium atom has the highest ionization energy in the periodic table.